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| Nickel(II) Sulfate | |
|---|---|
-sulfate-hexahydrate-sample.jpg) |
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6SO4.png) |
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| IUPAC name | Nickel(II) sulfate, hexahydrate |
| Identifiers | |
| CAS number | [10101-97-0] (hexahydrate); [10101-98-1](heptahydrate); [7786-81-4] (anhydrous) |
| EINECS number | |
| RTECS number | QR9600000 |
| Properties | |
| Molecular formula | NiSO4·6H2O |
| Appearance | Blue crystals (hexahydrate) |
| Density | 2.07 g/cm3 (hexahydrate) |
| Melting point |
decomp. >100 °C |
| Solubility in water | 775 g/L (30 °C) |
| Solubility in ethanol | sparingly (hexahydrate) |
| Structure | |
| Crystal structure | tetragonal |
| Coordination geometry |
octahedral at Ni |
| Hazards | |
| MSDS | ScienceLab.com |
| EU classification | not listed |
| NFPA 704 |
 0
2
0
|
| R-phrases | 22-40-42/43-50/53 |
| S-phrases | 22-36/37-60-61 |
| Related compounds | |
| Other anions | Nickel(II) bromide Nickel(II) chloride |
| Other cations | Copper(II) sulfate Cobalt(II) sulfate |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox references |
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Nickel(II) sulfate, or just nickel sulfate, usually refers to the chemical compound with the formula NiSO4·6H2O. This highly soluble blue-coloured salt is a common source of the Ni2+ ion for electroplating.
Several sulfate salts of nickel(II) are known, all being paramagnetic. These salts differ with respect to their hydration or subtle structural details. The common tetragonal hexahydrate crystallizes from aqueous solution between 30.7 and 53.8 °C. Below these temperatures, a heptahydrate crystallises and above these temperatures an orthorhombic hexahydrate forms. The yellow anhydrous form, NiSO4, is a high melting solid. This material produced by heating the hydrates above 330 °C. It decomposes at still higher temperatures to nickel oxide.1
X-ray crystallography measurements show that NiSO4·6H2O consists of octahedral [Ni(H2O)62+ ions. These ions in turn are hydrogen bonded to sulfate ions.2 Dissolution of the salt in water gives solutions containing the ion [Ni(H2O)62+.
Contents |
Production, applications, and coordination chemistry
The salt is usually obtained by dissolution of nickel metal or nickel oxides in sulfuric acid. Approximately 10,000,000 kg were produced in 2005. It is mainly used to for electroplating of nickel.
Aqueous solutions of nickel sulfate reacts with sodium carbonate to precipitate nickel carbonate, a precursor to nickel-based catalysts and pigments. Addition of ammonium sulfate to concentrated aqueous solutions of nickel sulfate precipitates Ni(NH4)2SO4·6H2O. This blue-coloured solid is analogous to Mohr's salt, Fe(NH4)2SO4·6H2O.1
Aqueous solutions of NiSO4·6H2O and related hydrates react with ammonia to give [Ni(NH3)6SO4 and with ethylenediamine to give [Ni(H2NCH2CH2NH2)3SO4. The latter is occasionally used as a calibrant for magnetic susceptibility measurements because it has no tendency to hydrate.
Natural occurrence
Nickel sulfate occurs as the rare mineral retgersite, which is a hexahydrate. The second hexahydrate is known as nickelhexahydrite (Ni,Mg,Fe)SO4·6H2O. The heptahydrate, which is relatively unstable in air, occurs as morenosite. The monohydrate occurs as very rare mineral dwornikite (Ni,Fe)SO4·H2O.
Safety
Nickel salts are carcinogenic, and this salt is a skin irritant
References
- ^ a b K. Lascelles, L. G. Morgan, D. Nicholls, D. Beyersmann “Nickel Compounds” in Ullmann's Encyclopedia of Industrial Chemistry 2005 Wiley-VCH, Weinheim, 2005.
- ^ Wells, A. F. (1984). Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
Wikipedia content modification information:
- This page was last modified on 18 August 2008, at 12:54.
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